Textbook Question
Consider the mixture of propane, C3H8, and O2 shown here. (c) How many molecules of CO2, H2O, C3H8, and O2 will be present if the reaction goes to completion?
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Ch.3 - Chemical Reactions and Reaction Stoichiometry
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970
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Table of contents
- Ch.1 - Introduction: Matter, Energy, and Measurement111
- Ch.2 - Atoms, Molecules, and Ions166
- Ch.3 - Chemical Reactions and Reaction Stoichiometry138
- Ch.4 - Reactions in Aqueous Solution127
- Ch.5 - Thermochemistry104
- Ch.6 - Electronic Structure of Atoms109
- Ch.7 - Periodic Properties of the Elements107
- Ch.8 - Basic Concepts of Chemical Bonding102
- Ch.9 - Molecular Geometry and Bonding Theories120
- Ch.10 - Gases122
- Ch.11 - Liquids and Intermolecular Forces79
- Ch.12 - Solids and Modern Materials102
- Ch.13 - Properties of Solutions99
- Ch.14 - Chemical Kinetics153
- Ch.15 - Chemical Equilibrium83
- Ch.16 - Acid-Base Equilibria109
- Ch.17 - Additional Aspects of Aqueous Equilibria117
- Ch.18 - Chemistry of the Environment60
- Ch.19 - Chemical Thermodynamics109
- Ch.20 - Electrochemistry113
- Ch.21 - Nuclear Chemistry79
- Ch.22 - Chemistry of the Nonmetals52
- Ch.23 - Transition Metals and Coordination Chemistry57
- Ch.24 - The Chemistry of Life: Organic and Biological Chemistry7
Brown15th EditionChemistry: The Central ScienceISBN: 9780137542970Not the one you use?Change textbook
Chapter 3, Problem 76a
Consider the mixture of propane, C3H8, and O2 shown here. (a) Write a balanced equation for the combustion reaction that occurs between propane and oxygen.
Verified step by step guidance1
Start by writing the unbalanced chemical equation for the combustion of propane: \( \text{C}_3\text{H}_8 + \text{O}_2 \rightarrow \text{CO}_2 + \text{H}_2\text{O} \)
Balance the carbon atoms first. Propane has 3 carbon atoms, so you need 3 \( \text{CO}_2 \) molecules: \( \text{C}_3\text{H}_8 + \text{O}_2 \rightarrow 3\text{CO}_2 + \text{H}_2\text{O} \)
Next, balance the hydrogen atoms. Propane has 8 hydrogen atoms, so you need 4 \( \text{H}_2\text{O} \) molecules: \( \text{C}_3\text{H}_8 + \text{O}_2 \rightarrow 3\text{CO}_2 + 4\text{H}_2\text{O} \)
Now, balance the oxygen atoms. You have 3 \( \text{CO}_2 \) molecules and 4 \( \text{H}_2\text{O} \) molecules, which means you need a total of 10 oxygen atoms (6 from \( \text{CO}_2 \) and 4 from \( \text{H}_2\text{O} \)): \( \text{C}_3\text{H}_8 + 5\text{O}_2 \rightarrow 3\text{CO}_2 + 4\text{H}_2\text{O} \)
Verify that all atoms are balanced: 3 carbon atoms, 8 hydrogen atoms, and 10 oxygen atoms on both sides of the equation.
Key Concepts
Here are the essential concepts you must grasp in order to answer the question correctly.
Combustion Reactions
Combustion reactions are chemical processes in which a substance reacts rapidly with oxygen, producing heat and light. In organic compounds like propane, the reaction typically produces carbon dioxide and water as products. Understanding the general form of combustion reactions is essential for writing balanced equations.
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Combustion Apparatus
Balancing Chemical Equations
Balancing chemical equations involves ensuring that the number of atoms of each element is the same on both sides of the equation. This is achieved by adjusting the coefficients of the reactants and products. A balanced equation reflects the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction.
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Stoichiometry
Stoichiometry is the quantitative relationship between reactants and products in a chemical reaction. It allows chemists to calculate the amounts of substances consumed and produced in a reaction. In the context of combustion, stoichiometry helps determine the precise ratios of propane and oxygen needed to achieve complete combustion.
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01:16Stoichiometry Concept
Related Practice
Textbook Question
The combustion of one mole of liquid octane, CH3(CH2)6CH3, produces 5470 kJ of heat. Calculate how much heat is produced if 1.000 gallon of octane is combusted.
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Textbook Question
Aluminum hydroxide reacts with sulfuric acid as follows: 2 Al1OH231s2 + 3 H2SO41aq2¡Al21SO4231aq2 + 6 H2O1l2 How many moles of the excess reactant remain after the completion of the reaction?
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Textbook Question
Consider the mixture of ethanol, C2H5OH, and O2 shown in the accompanying diagram. (c) How many molecules of CO2, H2O, C2H5OH, and O2 will be present if the reaction goes to completion?
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Textbook Question
Consider the mixture of ethanol, C2H5OH, and O2 shown in the accompanying diagram. (b) Which reactant is the limiting reactant?
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Textbook Question
Aluminum hydroxide reacts with sulfuric acid as follows: 2 Al1OH231s2 + 3 H2SO41aq2¡Al21SO4231aq2 + 6 H2O1l2 Which is the limiting reactant when 0.500 mol Al1OH23 and 0.500 mol H2SO4 are allowed to react?
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